To measure the amount of iron in a certain type of iron ore, an analytical chemist dissolves a sample in strong acid and titrates it to the endpoint with of potassium permanganate solution. The balanced chemical equation for the reaction is:

Explanation:

Hello!

In this case, for the described chemical reaction, we find it is:

Because it says that the iron is dissolved in a strong acid which provides addition hydrogen ions to the reaction media. Thus, for the questions attached on the figure we find:

- This a REDOX reaction because we see iron is being oxidized from 2+ to 3+ and manganese reduced from +7 to +2.

- Since it is a redox reaction and the oxidized species is that undergoing an oxidation number increase, we evidence iron goes from +2 to +3, which means iron is the oxidized species.

- In this case, for the used 59.2 mL (0.0592 L) of the 0.2000 M solution of potassium permanganate, we can compute the consumed grams of iron via stoichiometry including the 5:1 mole ratio between them in the chemical reaction:

It means that the percent of iron in that sample is:

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